3. The two molecules shown below have the same number of carbon atoms. Which do you think will have the larger standard molar entropy? Choose one from the descriptions below. Hint: we did not specifically discuss this in class, but use your knowledge of "disorder" to choose the most sensible answer. You can also do further research on the web. n-hexane iii. iv. V. cyclohexane i. n-hexane, because it has more hydrogen atoms (C6H14) than cyclohexane (C6H12). ii. cyclohexane, because it has fewer hydrogen atoms than n-hexane. They are the same because they have the same number of carbon atoms. n-hexane because it is less rigid than cyclohexane. cyclohexane, because it is more rigid than n-hexane.

3. The two molecules shown below have the same number of carbon atoms. Which do you think will have the larger standard molar entropy? Choose one from the descriptions below. Hint: we did not specifically discuss this in class, but use your knowledge of "disorder" to choose the most sensible answer. You can also do further research on the web. n-hexane iii. iv. V. cyclohexane i. n-hexane, because it has more hydrogen atoms (C6H14) than cyclohexane (C6H12). ii. cyclohexane, because it has fewer hydrogen atoms than n-hexane. They are the same because they have the same number of carbon atoms. n-hexane because it is less rigid than cyclohexane. cyclohexane, because it is more rigid than n-hexane.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. System A few grams of liquid water (H₂O). A few moles of helium (He) gas. A few moles of carbon dioxide (CO₂) gas. Change The water is cooled from 65.0 °C to -3.0 °C. The helium is heated from -4.0 °C to 69.0 °C while the volume is held constant at 10.0 L. The carbon dioxide is heated from 1.0 °C to 21.0 °C and is also compressed from a volume of 9.0 L to a volume of 6.0 L. AS AS 0 not enough information AS 0 not enough information AS 0 not enough information
4. Which of the following processes will have the largest positive value for the entropy change in the surroundings? ASsume state 1 has higher pressure and lower temperature than does state 2, and both states contain 1.00 mole of a monatomic perfect gas. a. a reversible process from state 1 to state 2 b. an irreversible process from state 1 to state 2 c. a reversible process from state 2 to state 1 d. an irreversible process from state 2 to state 1 e. cannot be determined from the information given
[References) Use the References to access important values if needed for this question. Arrange the following from lowest to highest entropy: CS2 (2), CS2 (g), CCL (g), S(s). Assume 1 mole of each at the same condit from lowest to highest entropy Drag and drop your selection from the following list to complete the answer: CS (g) S(s) CCL (g) CS2 () Submit Answer Try Another Version 2 item attempts remaining
Which of the following statements is TRUE regarding entropy? a. The entropy of the universe decreases after the occurrence of a spontaneous change. b. The entropy of any substance at temperatures above absolute zero is positive. c. The entropy is zero for a pure, perfect crystal at 0 °C. d.It is possible to determine the standard molar entropy of substances due to the second law of thermodynamics.
6) Which statement below best describes the Second Law of Thermodynamics? a. A perfectly ordered crystalline solid at zero Kelvin has zero entropy. b. The total entropy is positive for a spontaneous process. c. Energy is conserved. Scanned with CamScanner
At 363 K, one state is twice as likely as the other. The first (more likely) state has an energy of 9.19 kcal/mol and an entropy of 0.915 kcal/mol-K. The other state has an energy of 2.19 kcal/mol more then the first state. What is the entropy of the second (less likely) state?
For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S , or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. System Change S A few moles of carbon dioxide (CO2) gas. The carbon dioxide is heated from 9.0 °C to 36.0 °C and also expands from a volume of 6.0 L to a volume of 14.0 L. <S0 =S0 >S0 not enough information A few moles of helium (He) gas. The helium expands from a volume of 9.0 L to a volume of 15.0 L while the temperature is held constant at 20.0 °C. <S0 =S0 >S0 not enough information A few grams of liquid ammonia (NH3). The ammonia is heated from -1.0 °C to 2.0 °C. <S0…
For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. System A few grams of ammonia vapor (NH3). A few moles of nitrogen (N₂) gas. A few moles of nitrogen (N₂) gas. Change The ammonia condenses to a liquid at a constant temperature of -8.0 °C. The nitrogen is cooled from 78.0 °C to 3.0 °C while the volume is held constant at 2.0 L. The nitrogen is heated from -16.0 °C to 12.0 °C and also expands from a volume of 1.0 L to a volume of 10.0 L. AS AS 0 not enough information AS 0 O not enough information O AS 0 not enough information Ś
For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. System A few moles of carbon dioxide (CO₂) gas. A few grams of liquid ammonia (NH3). A few moles of carbon dioxide (CO₂) gas. Change The carbon dioxide expands from a volume of 10.0 L to a volume of 13.0 L while the temperature is held constant at 57.0 °C. The ammonia evaporates at a constant temperature of 11.0 °C. The carbon dioxide is cooled from 87.0 °C to -2.0 °C and is also expanded from a volume of 8.0 L to a volume of 11.0 L. AS AS 0 not enough information AS 0 not enough information AS 0 not enough information
Compare the compounds in each set below and decide which is expected to have the higher entropy. Assume all are at the same temperature. a. NH3 (g), ASH3 (g), or PH3 (g) O ASH3 (g) Ο ΝH: (g) O PH3 (g) b. NaCl(s) or NaCl(aq) O NaCl(aq) O NaCI(s) c. C2H4 (g) or N2 (g) (two substances with the same molar mass) ON2 (g) O C,H4 (g) d. C2H; OH(€) or C2H; OH(g) O C, H; OH(g) O C,H,OH(e)
For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. System A few moles of helium (He) gas. A few moles of carbon dioxide (CO₂) gas. A few moles of carbon dioxide (CO₂) gas. Change The helium is compressed from a volume of 11.0 L to a volume of 4.0 L while the temperature is held constant at -6.0 °C. The carbon dioxide is heated from -17.0 °C to 53.0 °C while the volume is held constant at 8.0 L. The carbon dioxide is heated from -8.0 °C to 3.0 °C and also expands from a volume of 10.0 L to a volume of 12.0 L. x AS AS 0 not enough information O AS 0 not enough information O AS 0 not enough information
8. You have discovered a new polymer. A monomer is shown below. To better understand its behavior you calculate its theoretical entropy. With careful measurements you find that it can be in 3 positions around the 1st bond in the chain, 2 around the 2nd bond, 1 around the 3rd bond and 3 around the 4th bond. Further, the ring can be in 4 different positions. What is the entropy in units of KB?